An investigation of neutralization reactions
Aim
Question :
What is the effect of changing the concentration of an alkali, on the volume of acid needed to neutralise it, when acid is added to it?
The plan is to use two acids (Hydrochloric & Sulphuric) and one alkali
(Sodium Hydroxide). The reason I need to use two acids is; because the question applies to all acids and alkalis and to just use one of each would not enable me to come to a general conclusion. If there had been more time available, ideally I would have preferred to use two alkalis as well as two acids.
Predictions
First of all, here are the definitions for an acid and an alkali:
An acid is a substance that forms hydrogen (H+) ions when placed in
water.
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Acids, which form one H+ ion from each acid molecule, are called Monoprotic. Acids, which form two, are called Diprotic. Acids, which form three, are called Triprotic (e.g. Orthophosphoric Acid [H3PO4])
I predict that for Monoprotic acids (e.g. Hydrochloric) :
Concentration of Acid * Volume of Acid = Concentration of Alkali *
Volume of Alkali
The amount of acid needed to neutralise an alkali =
(MAl * VAl)/MA = (Molarity of Alkali * Volume of Alkali)/Molarity of
Acid
I predict that for Diprotic acids (e.g. Sulphuric) :
Concentration of Acid * Volume of Acid = Concentration of Alkali *
Double the Volume of Alkali
Molarity = how many molecules of the acid or alkali per 1000 cm3 (1 litre) of water.
Equipment
Goggles (to protect the eyes)
Mat (to protect the surface of the bench)
Burette (to hold the acid)
Conical Flasks (to hold the alkali)
Indicator (to show the pH of the solution)
Funnel (to pour the acid into the burette)
Measuring Cylinders (to measure out the water, acid & alkali and
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On my graphs, since 0 concentration of Alkali will mean 0 volume of
Acid, I decided that the best fit line should carry on down to the origin. Because there were no data there, I had to extrapolate the line downwards and because of this it is shown as a red dotted line.
The data must be slightly inaccurate because the best fit line passes very close to the origin rather than actually passing through it.
Improvements
If this experiment was used again, I would try to improve it in the following ways :
* Instead of using Universal Indicator, I would use an indicator which only changed colour when the solution was Neutral rather than gradually changing as the pH became lower (e.g. Methyl Orange or Phenolphthalein).
* To get the pH more accurate next time, a pH meter could be used.
* To get it very accurate, the acids and alkalis supplied should be an exact amount (I am not sure whether the ones I used
In the pH homeostasis lab, 6 experiments were conducted. The hypotheses were: If base is added to water then the pH will increase; If acid is added to water then the pH will decrease; If base is added to homogenate, then the pH will increase; If acid is added to homogenate, then the pH will decrease; If acid or base is added to buffer, then the pH will remain the same. After the experiments were conducted, the graphs were somewhat similar to the hypotheses.
neutralize 35ml of our base. Once we weighed out the KHP we then dissolved it
Purpose/Introduction: In this experiment, four elimination reactions were compared and contrasted under acidic (H2SO4) and basic (KOC(CO3)3) conditions. Acid-catalyzed dehydration was done on 2-butanol and 1-butanol; a 2o and 1o alcohol, respectively. The base-induced dehydrobromination was performed on 2-bromobutane and 1-bromobutane isomeric halides. The stereochemistry and regiochemistry of the four reactions were analyzed by gas chromatography (GC) to determine product distribution (assuming that the amount of each product in the gas mixture is proportional to the area under its complementary GC peak).
· Wear the lab coat all the time in case the acid spills on you.
ranging from 50 cm³ of acid and no water, to 12.5 cm³ of acid and 37.5
Planning Firstly here is a list of equipment I used. Boiling tubes Weighing scales Knife Paper towels 100% solution 0% solution (distilled water) measuring beakers potato chips Cork borer. We planned to start our experiment by doing some preliminary work. We planned to set up our experiment in the following way.
Theories have often been developed to explain how delinquents violate social norms and still manage to maintain positive self images of themselves. Neutralization theory, developed by Gresham Sykes and David Matza in 1957 set out to do just this. Critics, however, have claims that the theory, on it’s own, is not a sufficient explanation for adolescent’s participation in crime in delinquency. It has also been claimed by critics that neutralization theory is best viewed as a components of larger theory of crime and can be incorporated into other theories such as social bond theory.
acids. I only tried the 1 molar acid, but if I were to repeat the
From looking at the results I can conclude that when the pH was 3 and
The Effect of Sodium Thiosulphate Solution on the Rate of its Reaction with Hydrochloric Acid
Neutralization Experiment AIM:- To investigate how heat is given out in neutralizing sodium hydroxide (NaOH) using different concentrations of Hydrochloric Acid. Background Information:- Substances that neutralize acids are called alkalis. An acid is a substance that forms hydrogen ions (H+ ) when placed in water. It can also be described as a proton donor as it provides H+ ions. An example of an acid is hydrochloric acid (HCl), Sulphuric acid (H2SO4) etc.
I decided to experiment with pHs within the range pH 2 to pH7, as I
viii. The experiment could have been performed over one a longer period of time day (rather than 14 days), which would have greatly reduced any loss of water from the sodium hydroxide solution, which may have improved results slightly.
* Concentration - I will try my best to use all the acid from the
0.1M HCl, 10 mL of 0.1N KMnO4, 0.2 g. KI, 5 mL of alcohol, and 5 mL of